Dependence of Reaction Rate On Concentration of Reactants

_____ (Law of mass action/Rate law) is an equation which represents the ratio between the masses of products and masses of reactants whose power is raised according to their stoichiometric coefficients.

Rate law expression is experimentally obtained, while law of mass action is theoretically obtained.

Rate law expression is theoritically obtained, while law of mass action is experimentally obtained.

State law of mass action.

Law of mass action states that the rate of any chemical reaction is proportional to the product of the masses of the reacting substances, with each mass raised to a power equal to the coefficient that occurs in the chemical equation. 

Law of _____ (conservation of mass/mass action) states that the rate of any chemical reaction is proportional to the product of the masses of the reacting substances, with each mass raised to a power equal to the coefficient that occurs in the chemical equation. 

The units of rate constant is same as that of rate. The order of the reaction is:

Rate law cannot be determined from balanced chemical equation if _____.

Rate law cannot be determined from balanced chemical equation if _______.

The rate of reaction, $\mathrm{A}\to$ Products is $1.25\times {10}^{-2}\mathrm{M}/\mathrm{s}$ when concentration of $\mathrm{A}$ is $0.45\mathrm{M}$. Determine the rate constant if the reaction is second order in $\mathrm{A}$.

The following results were obtained in the decomposition of H2O2 in KI solution at 30°C

Show that the reaction is first order. Calculate the rate constant of the reaction.

From the following data for the liquid phase reaction $\mathrm{A} \to \mathrm{B}$, determine the order of the reaction and calculate its rate constant.

For the reaction, ${\mathrm{A}}_2+\mathrm{B}+\mathrm{C}⟶\mathrm{AC}+\mathrm{AB},$ it is found that tripling the concentration of ${\mathrm{A}}_2$ triples the rate, doubling the concentration of $\mathrm{C}$ doubles the rate and doubling the concentration of $\mathrm{B}$ has no effect.

Why the change in concentration of $\mathrm{B}$ has no effect?

For the reaction, ${\mathrm{A}}_2+\mathrm{B}+\mathrm{C}⟶\mathrm{AC}+\mathrm{AB},$ it is found that tripling the concentration of ${\mathrm{A}}_2$ triples the rate, doubling the concentration of $\mathrm{C}$ doubles the rate and doubling the concentration of $\mathrm{B}$ has no effect.

What is the rate law?

Comment on the relationship between coefficients of the balanced overall equation for a reaction and the exponents to which the concentration terms in the rate law are raised. What do these exponents represent?

Write the rate law for the following reaction:
A reaction that is second order in $\mathrm{NO}$ and first order in ${\mathrm{Br}}_2.$
 

For the reaction $2\mathrm{A} + \mathrm{B} \to$ products, find the rate law from the following data

What is the rate constant and order of the reaction?
 

Consider the reaction $2\mathrm{A} + 2\mathrm{B} \to 2\mathrm{C} + \mathrm{D}$. From the following data, calculate the order and rate constant of the reaction.

Write the rate law of the reaction.

The reaction $\mathrm{A}+\mathrm{B}\to$ products is first order in each of the reactants.

What is the change in the rate if concentration of $\mathrm{A}$ is doubled and that of $\mathrm{B}$ is halved ?

The reaction $\mathrm{A}+\mathrm{B}\to$ products is first order in each of the reactants.

What is the change in the rate if the concentration of each reactant is tripled?